Calculate the molar mass of a gas if 4.40g occupies at 3.50 L at 560mmHg and 41 degrees celsisus
PV = nRT and solve for n = mols.
Then mols = grams/molar mass. You have mols and grams, solve for molar mass. Remember K must be in kelvin and P must be in atm if you use R as 0.08206
Solution please im confused
pv=nRT
n=PV/RT
n=0,7368x3500/0,8206x314
n=10
Mr=4,40/10
=0,44
To calculate the molar mass of a gas, we need to use the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the given temperature from Celsius to Kelvin. To convert Celsius to Kelvin, we add 273.15 to the Celsius temperature. In this case, the given temperature is 41 degrees Celsius, so we have:
T (in Kelvin) = 41 + 273.15 = 314.15 K
Now, let's convert the given pressure from mmHg to atm. The conversion factor is 1 atm = 760 mmHg. Thus, 560 mmHg is equal to:
Pressure (in atm) = 560 mmHg / 760 mmHg/atm = 0.737 atm
Next, we can rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT
n = (0.737 atm) * (3.50 L) / [(0.0821 L·atm/mol·K) * (314.15 K)]
n ≈ 0.1003 moles
Now that we have the number of moles, we can calculate the molar mass (M) of the gas using the given mass (4.40 g) and the number of moles:
M = mass / moles
M = 4.40 g / 0.1003 moles
M ≈ 43.93 g/mol
Therefore, the molar mass of the gas is approximately 43.93 g/mol.